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Compare the size of cations and anions to their parent atoms.
Cations: Smaller than their parent atoms. Anions: Larger than their parent atoms.
Compare the electrical conductivity of ionic compounds in solid vs. liquid/aqueous states.
Solid: Poor conductors. Liquid/Aqueous: Good conductors.
Compare the lattice energy of NaF vs. NaCl. Explain why.
NaF has a higher lattice energy because $F^-$ is smaller than $Cl^-$.
Compare the lattice energy of MgO vs. NaF. Explain why.
MgO has a higher lattice energy because $Mg^{2+}$ and $O^{2-}$ have higher charges than $Na^+$ and $F^-$.
Compare the lattice energy of LiCl vs. NaCl. Explain why.
LiCl has a higher lattice energy because $Li^+$ is smaller than $Na^+$.
What effect does a higher charge have on lattice energy?
Higher charges lead to higher lattice energy.
What effect does a smaller distance between ions have on electrostatic force?
Smaller distances lead to stronger electrostatic force.
What happens when an ionic compound is in the liquid or aqueous state?
Ions are delocalized and can carry a charge, making the compound a good conductor of electricity.
What causes ionic compounds to have high melting and boiling points?
Strong electrostatic forces require a lot of energy to overcome, resulting in high melting and boiling points.
What is the effect of ionic compounds having strong forces?
Makes it difficult to deform the solid, but the lattice can easily shatter.
Define 'cation'.
A positively charged ion formed when a metal loses electrons.
Define 'anion'.
A negatively charged ion formed when a nonmetal gains electrons.
What is a crystal lattice?
A 3-D array formed by ionic compounds, maximizing attractive forces and minimizing repulsive forces.
Define 'lattice energy'.
The energy released when ions combine to form an ionic solid; a measure of the strength of ionic bonds.
What is Coulomb's Law?
Describes the electrostatic force between ions: $F = k \frac{q_1 q_2}{r^2}$, where F is the force, k is Coulomb's constant, q1 and q2 are the charges, and r is the distance.